Question

Would a reaction occur if solid tin was placed in a solution of copper (II) nitrate?

If so, what is the balanced net ionic equation for the reaction?

Answer 1

No because....

Explanation:

Tin is less reactive and can not displace copper..

Answer 2

Of course a reaction would occur

Explanation:

As the standard reduction potential of copper is higher than tin, it will get reduced.

Net reaction is:

`Cu(NO_3)_2 + Sn rarr Sn(NO_3)_2 + Cu`

Answer 3

The single replacement reaction will occur.

The net ionic equation is:

`"Sn(s) + Cu"^(2+)("aq")"` `rarr` `"Cu(s) + Sn"^(2+)("aq")"`

Explanation:

In order to determine whether a reaction will occur we need to consult a reactivity series of metals like the one below. In a single replacement reaction can occur only if the metal reactant, in this case tin (Sn) is more reactive than the metal in the reactant that is a compound, in this case copper (Cu). As you can see, tin is above copper in the reactivity series, so this reaction will occur.

Balanced molecular equation

`"Sn(s) + Cu(NO"_3)_2("aq")"` `rarr` `"Cu(s) + Sn(NO"_3)_2("aq")"`

Complete ionic equation

`"Sn(s) + Cu"^(2+)("aq") + "2NO"_3("aq")"` `rarr` `"Cu(s) + Sn"^(2+)("aq") + "2NO"_3("aq")"`

Net ionic equation

Remove the ions that occur on both sides of the equation.

`"Sn(s) + Cu"^(2+)("aq")"` `rarr` `"Cu(s) + Sn"^(2+)("aq")"`